Is the question formulating correctly? If yes, return the question without changes. If not, please fix it and return the output as a JSON of the form: {'question': 'question text'}. Here is the question: Make a sketch of the voltaic cell represented by the line notation. Write the overall balanced equation for the reaction and calculate E°cell. Mn(s) | Mn2+(aq) || ClO2-(aq) | ClO2(g) | Pt(s)

Verified step by step guidance

1. Step 1: Identify the components of the voltaic cell from the line notation. The notation 'Mn(s) | Mn^{2+}(aq) || ClO_2^-(aq) | ClO_2(g) | Pt(s)' indicates that manganese is the anode and the chlorine dioxide is the cathode.
2. Step 2: Write the half-reactions for the anode and cathode. For the anode, the oxidation reaction is Mn(s) → Mn^{2+}(aq) + 2e^-. For the cathode, the reduction reaction is ClO_2(g) + e^- → ClO_2^-(aq).
3. Step 3: Balance the electrons in the half-reactions. Multiply the cathode half-reaction by 2 to balance the electrons: 2(ClO_2(g) + e^- → ClO_2^-(aq)).
4. Step 4: Combine the balanced half-reactions to write the overall balanced equation for the cell reaction. Add the balanced half-reactions together, ensuring that the electrons cancel out.
5. Step 5: Calculate the standard cell potential, E°_{cell}, using standard reduction potentials from a table. Use the formula E°_{cell} = E°_{cathode} - E°_{anode} to find the cell potential.